Photosynthesis in plants converts carbon dioxide and water into glucose (C,H12O) and oxyge-according to the equation below.1.6CO,(g) + 6H,0(1)CH1,0(s) + 60,(g)SubstanceCO,(g)H,O()C,H12O6ls)Ozlg)AH?(kJ/mol)-393.5-285.8-1 273.3S°J/mol · K)213.669.9209.2205.0Calculate the AH°, Asº, and AGº. Is the reaction spontaneous at standard conditions?

Answered: Image /qna-images/answer/745afc9a-1680-40ca-abc2-0ccba54706cf.jpg

Photosynthesis in plants converts carbon dioxide and water into glucose (C,H1¿O¿) and according to the equation below. oxyge 6CO,(g) + 6H,O(1) CH1,O(s) + 60,(g) Substance CO,(g) H,O() C,H12O6ls) Ozlg) AH?(kJ/mol) -393.5 - 285.8 -1 273.3 S°U/mol · K) 213.6 69.9 209.2 205.0 Calculate the AH°, Asº, and AG°. Is the reaction spontaneous at standard conditions?

Photosynthesis in plants converts carbon dioxide and water into glucose (C,H1¿O¿) and according to the equation below. oxyge 6CO,(g) + 6H,O(1) CH1,O(s) + 60,(g) Substance CO,(g) H,O() C,H12O6ls) Ozlg) AH?(kJ/mol) -393.5 - 285.8 -1 273.3 S°U/mol · K) 213.6 69.9 209.2 205.0 Calculate the AH°, Asº, and AG°. Is the reaction spontaneous at standard conditions?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the AH°, for the reaction below, in kJ, using the heat of formation values below: _X4Y2 (g) + Z, (g)→ --_X2Z4 (g) + LY4Z2 () AH°; [X4Y2 (g)] = -300.5 kJ/mol AH°; [Z, (g)] = O k//mol AH°; [X2Z4 (g)] = -110.4 kJ/mol AH°; [Y4Z2 (] = 278.9 kJ/mol %3D HINT: Balance the reaction FIRST!
Please help me solve the given question, explain and make sure its 100% correct ! Greatly appreciate it
4. Use Hess's Law and the following data; CHale) + 202) CO2le) + 2H,0(g) AH = - 802 KJ + CO2(e) 2C0 + 2H2g) AH = + 247 KJ CH416) + H,0e) + 3H2(e) AH = + 206 KJ + To determine AH for reaction: CH4le) + % Ozle) » COe) + 2H2e)
Use the standard reaction energies given below to determine AGºrxn for the following reaction: XY4(g) + Y2O(g) --> XO(g) + 3Y2(g) Given: 2Y2(g) + XO(g) - --> XY3OY(1) DG-134.32 kJxmol-1 2XY4(g) + O2(g) - --> 2XY3OY(1) DG-133.11 kJxmol-1 2Y2(g) + O2(g) --> 2Y2O(g) DH-190.99 kJxmol-1 Give answer in KJ/mol. Give answer to two decimal places. Do not include units in answer. Your Answer:
Pls help ASAP
Use your table of Heats of Formation to calculate the heat of reaction for the following reaction: C2H4(g) + 3O2(g) ⟶ 2CO2(g) + 2H2O(g)
How do I find the kJ?
11. answer question in pic pls
Calculate AHrxn for the reaction below. 2 NOCI(g) → N2(g) + 02(g) + Cl2(9) You are given the following set of reactions. 1/2 N2(g) + 1/2 02(g) → NO(g) AH = 90.30 k) NO(g) + 1/2 Cl2(g) → NOCI(g) AH = -38.6 kJ 4.0 kJ
21. The enthalpy changes of these reactions can be measured: AH° = -1411.1 kJ C,H,(g) +30,(g) C,H,OH(C) + 3 0,(g) 2 CO,(g) +2 H,O(€) 2 CO,(g) + 3 H,0(e) 1) AH° =-1367.5 kJ - Use these values and Hess's law to determine the enthalpy change for the reaction CH,(g) + H,0(() CH,OH(€)
Per x M Inb x 31799#/7231799/2/0 ted 13 out of 16 16 P11 Essentials of General, Organic, and Biochemistry Denise Guinn THIRD EDITION The table lists the specific heat values for brick, ethanol, and wood. Specific Heats of Substances Substance Brick Ethanol Wood heat added: P S per: X 20 effe x CDC He: X JA 6 Specific Heat 0.20 0.58 0.10 B 10 X 4 gºC Calculate the amount of heat, in calories, that must be added to warm 96.8 g of brick from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. W 4 Calculate the amount of heat, in calories, that must be added to warm 96.8 g of ethanol from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. ○바 8 No X 9 EC eth X 0 Sm X 00 39 HR MIN SEC 0/R Sm x Resources + presented by Macmillan Learning G ا ا ا 200 L Next Qu cal 40 1
The value of AH° for the reaction below is -6535 kJ. ob kJ of heat are released in the combustion of 16.0 g of C6H6 (1)? MM C6H6 = 78.12 g/mol 2C6H6 (1) + 1502 (g) → 12CO2 (g) + 6H₂O (1) 1 A) 669 SHAHB)-6535 C) 1.34 x 103 D) 5.23 x 104 E) 2.68 x 103 Only typed solution.